Predict the direction of the net reaction as a result of increasing the pressure (decreasing the volume) on the system at constant temperature in the following equilibrium system; 2NO (g) + H2 (g) N20 (g) + H20 (g) The net reaction will shift towards the reactants (to the left) when pressure is increased Change in pressure has no effect on the equilibrium The net reaction will shift towards the products (to the right) when pressure is increased None of the above

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Chapter1: Chemical Foundations
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**Title: Predicting the Direction of Reaction for Pressure Changes in Equilibrium Systems**

**Objective:**
Understand how changes in pressure influence the direction of a chemical reaction at equilibrium.

**Equilibrium Reaction System:**

\[ 2 \text{NO} \, (g) + \text{H}_2 \, (g) \rightarrow \text{N}_2\text{O} \, (g) + \text{H}_2\text{O} \, (g) \]

**Question:**
Predict the direction of the net reaction as a result of increasing the pressure (decreasing the volume) on the system at constant temperature.

**Answer Choices:**

- **Option A:** The net reaction will shift towards the reactants (to the left) when pressure is increased.
- **Option B:** Change in pressure has no effect on the equilibrium.
- **Option C:** The net reaction will shift towards the products (to the right) when pressure is increased.
- **Option D:** None of the above.

**Concept Explanation:**

In systems at equilibrium, increasing the pressure generally causes the reaction to favor the side with fewer moles of gas. This is due to Le Chatelier's principle, which states that a system will adjust to counteract the effect of a change. Therefore, for the given reaction:

- **Reactants:** \(2 \text{NO} \, (g) + \text{H}_2 \, (g)\) (3 moles of gas)
- **Products:** \(\text{N}_2\text{O} \, (g) + \text{H}_2\text{O} \, (g)\) (2 moles of gas)

When the pressure is increased, the equilibrium will shift toward the side with fewer moles of gas, which is the **products** side.

**Correct Answer:**
Option C: The net reaction will shift towards the products (to the right) when pressure is increased.
Transcribed Image Text:**Title: Predicting the Direction of Reaction for Pressure Changes in Equilibrium Systems** **Objective:** Understand how changes in pressure influence the direction of a chemical reaction at equilibrium. **Equilibrium Reaction System:** \[ 2 \text{NO} \, (g) + \text{H}_2 \, (g) \rightarrow \text{N}_2\text{O} \, (g) + \text{H}_2\text{O} \, (g) \] **Question:** Predict the direction of the net reaction as a result of increasing the pressure (decreasing the volume) on the system at constant temperature. **Answer Choices:** - **Option A:** The net reaction will shift towards the reactants (to the left) when pressure is increased. - **Option B:** Change in pressure has no effect on the equilibrium. - **Option C:** The net reaction will shift towards the products (to the right) when pressure is increased. - **Option D:** None of the above. **Concept Explanation:** In systems at equilibrium, increasing the pressure generally causes the reaction to favor the side with fewer moles of gas. This is due to Le Chatelier's principle, which states that a system will adjust to counteract the effect of a change. Therefore, for the given reaction: - **Reactants:** \(2 \text{NO} \, (g) + \text{H}_2 \, (g)\) (3 moles of gas) - **Products:** \(\text{N}_2\text{O} \, (g) + \text{H}_2\text{O} \, (g)\) (2 moles of gas) When the pressure is increased, the equilibrium will shift toward the side with fewer moles of gas, which is the **products** side. **Correct Answer:** Option C: The net reaction will shift towards the products (to the right) when pressure is increased.
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